I know the correct answer is B and also that there is a explanation below it. But can someone explain this in more simpler terms Iâm having trouble understanding why B is the correct answer
MS-3.. The fact that BCl, is a planar molecule while NCI, is pyramidal can be explained several different ways. Which statement is the best rationalization? (A) Nitrogen is more electronegative than boron. (B) The nitrogen atom in NCl, has a lone pair of electrons, whereas the boron atom in BCl, does (C) The nitrogen atom is smaller than the boron atom. (D) The boron atom in BCl, is sp' hybridized, while the nitrogen atom in NCl, is sp' hybridized. not. nowledge Required: (1) The valence-shell-electron-pair-repulsion (VSEPR) model for predicting molecular hape. (2) The valence-bond theory for predicting hybridization of orbitals. hinking it Through: Choices (A) and (C) are both true statements, but neither provides the reason for the ference in geometries. The VSEPR model does provide a rationalization for the difference. Choice (D) has the bridization reversed. NCl, has an sp hybridized nitrogen atom, and BCl, has an sp hybridized boron atom. oice (B), the correct answer, recognizes that boron has only enough valence electrons to form three bonds, wit lone pairs. The six electrons arrange themselves to have 120° Cl-B-Cl bond angles. On the other hand, when l, forms three bonds it has an electron pair left over to complete the octet. The four electron pairs arrange mselves in the shape of a tetrahedron around the nitrogen atom. Here are the Lewis structures and their three- ensional representations: :CI: CI:B:CI Cl :ci: 120° N, 109° Cl
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